Chemistry Solutions and Molarity Quiz

A homogeneous mixture of two or more components. The component present in lesser amount is called solute and the component present in larger amount is called solvent.

A solution made up of two components.

A solution made up of three components.

A solution made up of four components.

A solution where water is present in excess.

A solution where water is not present in excess.

A method to express the concentration of a solution by calculating the ratio of the mass of a component to the total mass of the solution, multiplied by 100.

The concentration of a solution.

A measure of the concentration of a solute in a solution. It's defined as the moles of solute per kilogram of solvent.

A measure of how much mass is contained in a given volume. It's defined as mass per unit volume.

A measure of the concentration of a solute in a solution. It's defined as the moles of solute per liter of solution.

The mass of one mole of a substance. It's expressed in units of grams per mole (g/mol).

Conversion of Units: 1 mL = 1 cm³

A solution in which no more solute can be dissolved at a given temperature and pressure. It is a state of equilibrium where the rate of dissolution equals the rate of crystallization.

A solution in which more solute can be dissolved at the same temperature and pressure.

The process of dissolving a solid solute in a solvent to form a solution. The concentration of the solution increases as more solute dissolves.

The process where solute particles in a solution collide with the solid solute and separate out of the solution, forming crystals. This happens when the solution becomes saturated or if the temperature is lowered.

A state of dynamic equilibrium in a saturated solution where the rate of dissolution of solute particles equals the rate of crystallization of solute particles.

The amount of solute dissolved in a given amount of solvent at a specific temperature and pressure.

The mass of solute dissolved in 100g of solvent.

The mass of solute dissolved in 100mL of solvent.

A measure of the concentration of a solution expressed as the number of moles of solute per kilogram of solvent.

The unit used to measure the amount of a substance, equal to the molecular weight in grams.

The mass of one mole of a substance.

Henry's Law states that the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid. This means that the higher the partial pressure of the gas, the more soluble it will be.

A constant that relates the partial pressure of a gas to its solubility in a liquid at a given temperature. It is specific to each gas and solvent combination.

The partial pressure of a gas above a liquid is directly proportional to the mole fraction of the gas in the liquid. This relationship is used to calculate the solubility of a gas in a liquid.

The process of a gas dissolving into a liquid. The solubility of a gas is influenced by factors such as temperature, pressure, and the nature of the gas and solvent.

The total vapor pressure of a solution is determined by the partial pressures of its components. The vapor pressure of each component is proportional to its mole fraction in the solution. This relationship can be expressed by Raoult's Law, which states that the partial pressure of a component in an ideal solution is equal to the product of its mole fraction and its vapor pressure in the pure state.

In an ideal solution, the interactions between the different components are the same as the interactions between the same components. In a non-ideal solution, the interactions between the different components are different from the interactions between the same components. This difference can affect the vapor pressure, boiling point, and other properties of the solution.

The mole fraction of a component in a binary mixture is the ratio of the number of moles of that component to the total number of moles in the mixture.

The total vapor pressure of an ideal solution is a linear function of the mole fraction of each component. This means that the vapor pressure of the solution will be directly proportional to the amount of each component present.

The deviation from Raoult's Law can be positive, negative, or both. Positive deviations occur when the interactions between the different components are weaker than the interactions between the same components, resulting in a higher vapor pressure than predicted by Raoult's Law. Negative deviations occur when the interactions between the different components are stronger than the interactions between the same components, resulting in a lower vapor pressure than predicted by Raoult's Law.